A particular reaction is spontaneous upto 475k and becomes non-spontaneous at temperatures above 475k. (i) is this reaction exothermic or endothermic?
(ii) does entropy increase or decrease during the reaction?
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The reaction is exothermic and the entropy decreases during the reaction.
- We know that , ΔG=ΔH-TΔS
- A reaction is spontaneous if ΔG for the reaction is negative and the reaction is non-spontaneous if ΔG for the reaction is positive.
- The given reaction becomes non spontaneous with increase in temperature which indicates that ΔS of the reaction must be negative since only that will lead ΔG to become positive with increase in temperature.
- At lower temperature, the reaction is spontaneous which indicates that ΔH is negative and dominates over the positive (-TΔS) term until the temperature reaches 475 K.
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